A 150.0 ml container is filled with a mixture of oxygen and nitrogen to a pressure of 120 kPa at 28 oC. If the mixture of the gas has a weight of 1.2455 g, calculate the percentage mole of nitrogen in the gas mixture

Q: A sample of unknown gas has a mass of 2.85 g and occupies 750 mL at 760 mm Hg and 100 °C. What is…

A: Ideal gases have negligible volume in compare to the volume of the container and molecules of ideal…

Q: Calculate the total pressure (in atm) of a mixture of 0.0200 mol of He, and 0.100 mol of H2 in a…

A: Given, 0.0200 mol of He, and 0.100 mol of H2 in a 2.50 L flask at 10 °C

Q: A 3.40 gram mixture of potassium chlorate KCLO3, and potassium chloride, KCL, was heated until all…

A: Given, KClO3(s) ➝ KCl(s) + O2(g) Balancing the above equation, 2KClO3(s) ➝ 2KCl(s) + 3O2(g) Pressure…

Q: A mixture of Ne and Ar gases at a PT of 1.4atm. If there are twice as many mols of Ne as Ar, what is…

A: The mixture contains Ne and Ar in the ratio 2:1. Hence, mole fraction of Ar can be given as below,

Q: A 6.00 L tank at 12.2 °C is filled with 5.23 g of chlorine pentafluoride gas and 13.7 g of boron…

A: Ideal gas equation:  PV = nRT  P = Pressure V = Volume n = Total number of moles  R = Gas constant T…

Q: A 6.0-L flask contains a mixture of methane (CH4), argon, and helium at 45oC and 1.75 atm. If the…

A: Given information, A 6.0-L flask contains a mixture of methane (CH4), argon, and helium at 45oC and…

Q: The total pressure of a mixture of gas is 800 torr. What are the partial pressures of the component…

A: Number of moles can be calculated as follows: No. of moles of CO2 = massatomic mass = 80g44…

Q: What is the molar mass of a gas if a 0.227 g sample occupies 135 mL at 25 *C and 68.5 kPa? *

A: Ans is 60.81g/mol

Q: A 5.00 L tank at 12. °C is filled with 14.2 g of chlorine pentafluoride gas and 3.58 g of sulfur…

A:

Q: For a certain hydrocarbon gas, 20.0 mg exerts a pressure of 24.7 torr in a 500-cm3 vessel at 25…

A: Ideal gas equation is  PV =nRT  P = pressure of hydrocarbon gas = 24.7 torr = 0.0325 atm  V = volume…

Q: A 10.0 L tank at 0.86 °C is filled with 12.3 g of dinitrogen difluoride gas and 9.28 g of chlorine…

A: According to the question, The temperature of the tank is = T= 0.86°C = 273.15+0.86 K = 274.01 K The…

Q: A 10.0 L tank at 17. °C is filled with 9.03 g of dinitrogen monoxide gas and 6.93 g of chlorine…

A: Given that -  Volume of the tank = 10.0 L  Temperature = 17.0°C = 273+17 = 290 K  Weight of…

Q: 11.76 grams of nitrogen, 19.2 grams of oxygen and 3.6 grams of argon at a total pressure of 300 kPa.…

A:

Q: A 5.00 L tank at 4.58 °C is filled with 15.2 g of chlorine pentafluoride gas and 7.62 g of sulfur…

A: Ideal gas equation: PV = nRT  P = Pressure V = Volume n = Number of moles  R = Gas constant T =…

Q: What is the density, in grams per liter, of a gas with a molar mass of 17.02gmol at 303 K and 1.50…

A: We have to find  the density, in grams per liter, of a gas with a molar mass of 17.02g/mol at 303 K…

Q: Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the…

A:

Q: A 9.00 L tank at 12. °C is filled with 17.4 g of dinitrogen difluoride gas and 9.28 g of sulfur…

A:

Q: A 7.00 L tank at 9.47 °C is filled with 6.90 g of dinitrogen difluoride gas and 5.31 g of chlorine…

A:

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: Since you have posted questions with multiple subparts, we are entitled to answer the first 3 only.…

Q: A 9.00 L tank at 28.9 °C is filled with 8.24 g of sulfur tetrafluoride gas and 5.83 g of chlorine…

A: Volume of the tank = 9 LTemperature = 28.9 0CAmount of sulfur tetrafluoride = 8.24 gAmount of…

Q: 1. A sample of gas weighs 3.10 g and occupies a volume of 1,272 mL at 30 °C and 720 mm Hg. What is…

A: According to ideal gas law, PV = nRT where P = pressure in atm  V = volume in L n = moles R = gas…

Q: Calculate the density of sulfur hexafluoride gas at 703 torr and 21 °C. Express the density in grams…

A: Given, Gas = sulfur hexafluoride pressure =703 torr temperature =21°C=(21+273)K=294 K

Q: What is the volume of 0.188 moles of fluorine gas contained at 27.1oC with a pressure of 151.95 kPa?

A: According to ideal gas equation, the pressure, volume, the number of moles and the temperature are…

Q: Chlorine pentafluoride gas is collected at 9.0°C in an evacuated flask with a measured volume of…

A: Given :-  pressure of gas = 0.410 atm  volume occupied by gas = 5.0 L  temperature = 9.0°C  To…

Q: A 6.0-L flask contains a mixture of methane (CH₄), argon,and helium at 45°C and 1.75 atm. If the…

A: Ideal gas equation:                                                                      PV=nRT…

Q: A gas made up of atoms escapes through a pinhole 2.04 times as fast as Kr gas. Write the chemical…

A:

Q: A 1.00 m3 container holds a sample of O2 gas. At 287 K the pressure of the container is 1.06 x 105…

A:

Q: A 8.00 L tank at 4.12 °C is filled with 11.7 g of chlorine pentafluoride gas and 14.1 g of boron…

A: The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a…

Q: A mixture contains O2 at 700. torr pressure, F2 at 900. torr pressure, and Cl2 at 400. torr…

A: Given that, Pressure of O2=700 torr pressure of F2=900 torr pressure of Cl2=400torr then,

Q: A gas sample occupies 563 mL at 18.0 °C and 79.2 kPa. How many gas molecules are in the sample?

A: Given,  Volume = 563 mL  Temperature = 18.0 °C  Pressure = 79.2 kPa   To calculate : number of gas…

Q: What is the molar mass of a gas if a 0.227 g sample occupies 135 mL at 25 °C and 68.5 kPa?

A:

Q: A mixture of N2 and CO2 gases has an average molar mass of 32.8 g/mol. What is the partial pressure…

A:

Q: Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the…

A: Information about the question

Q: A tank contains a mixture of 55.5 % oxygen gas and 44.5 % carbon dioxide gas by mass at 27°C. The…

A: The partial pressure of a gas in a mixture of gases is the product of total pressure and mole…

Q: The mass of an evacuated 255 mL flask is 143.187 g. The mass of the flask filled with 267 torr of an…

A:

Q: partial pressure

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Q: "Calculate the total pressure of mixture of 1.31g of nitrogen gas. 2.53g of hydrogen gas, and 3.26g…

A:

Q: Imagine that you have a 6.50 LL gas tank and a 4.50 LL gas tank. You need to fill one tank with…

A:

Q: What is the partial pressure of neon that's 18% by volume in a gas mixture with a total pressure of…

A: Answer: According to Dalton's law of partial pressure, partial pressure of any gas in the gaseous…

Q: container was filled with 0.893 moles of N2, 0.687 moles of O2, 0.734 moles of H2, and 0.248 moles…

A:

Q: A 8.00 L tank at 18. °C is filled with 6.96 g of dinitrogen difluoride gas and 11.8 g of chlorine…

A: The total pressure present in the tank can be calculated using the ideal gas law equation which is…

Q: convert between them

A: In order to convert a pressure unit to another one, we need to know the relationship between these…

Q: A 2.00 m3 container holds a sample of O2 gas. At 287 K the pressure of the container is 1.04 x 105…

A: Given,  Volume of the container, V = 2.00 m3                                                 = 2000…

Q: A mixture contains O2 at 700. torr pressure, F2 at 600. torr pressure, and Cl2 at 400. torr…

A: Given that, PO2=700 torr, PF2=600 torr PCl2=400 torr

Q: A 8.00 L tank at 24.8 °C is filled with 4.16 g of chlorine pentafluoride gas and 11.6 g of sulfur…

A: The mass of Chlorine pentafluoride, ClF5 = 4.16 gThe mass of Sulfur hexafluoride, SF6 = 11.6 gThe…

Q: A 9.00 L tank at 7.61 °C is filled with 9.76 g of sulfur hexafluoride gas and 6.26 g of chlorine…

A: we have to calculate mole fraction, partial pressure of each gas and the total pressure in the tank

Q: A sample of CO2 occupies a volume of 14.87 liters at 140.5 kPa. What pressure in kPa would the gas…

A:

Q: A 5.00 L tank at 3.03 °C is filled with 14.4 g of chlorine pentafluoride gas and 7.02 g of sulfur…

A:

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.